US5739367A - Cobalt catalyst - Google Patents
Cobalt catalyst Download PDFInfo
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- US5739367A US5739367A US08/817,295 US81729597A US5739367A US 5739367 A US5739367 A US 5739367A US 81729597 A US81729597 A US 81729597A US 5739367 A US5739367 A US 5739367A
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- process according
- cobalt
- solution
- ammonia
- iii
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- 229910017052 cobalt Inorganic materials 0.000 title claims description 23
- 239000010941 cobalt Substances 0.000 title claims description 23
- GUTLYIVDDKVIGB-UHFFFAOYSA-N cobalt atom Chemical compound [Co] GUTLYIVDDKVIGB-UHFFFAOYSA-N 0.000 title claims description 22
- 239000003054 catalyst Substances 0.000 title description 5
- QGZKDVFQNNGYKY-UHFFFAOYSA-N Ammonia Chemical compound N QGZKDVFQNNGYKY-UHFFFAOYSA-N 0.000 claims abstract description 62
- 238000006243 chemical reaction Methods 0.000 claims abstract description 34
- 229910021529 ammonia Inorganic materials 0.000 claims abstract description 28
- 150000001868 cobalt Chemical class 0.000 claims abstract description 18
- 150000001412 amines Chemical class 0.000 claims abstract description 17
- 150000001450 anions Chemical class 0.000 claims abstract description 11
- JAWGVVJVYSANRY-UHFFFAOYSA-N cobalt(3+) Chemical compound [Co+3] JAWGVVJVYSANRY-UHFFFAOYSA-N 0.000 claims abstract description 10
- 229910052739 hydrogen Inorganic materials 0.000 claims abstract description 9
- 150000002500 ions Chemical class 0.000 claims abstract description 9
- XLJKHNWPARRRJB-UHFFFAOYSA-N cobalt(2+) Chemical compound [Co+2] XLJKHNWPARRRJB-UHFFFAOYSA-N 0.000 claims abstract description 7
- 125000001183 hydrocarbyl group Chemical group 0.000 claims abstract description 6
- 125000004432 carbon atom Chemical group C* 0.000 claims abstract description 5
- 239000001257 hydrogen Substances 0.000 claims abstract description 5
- 238000004519 manufacturing process Methods 0.000 claims abstract description 5
- UFHFLCQGNIYNRP-UHFFFAOYSA-N Hydrogen Chemical compound [H][H] UFHFLCQGNIYNRP-UHFFFAOYSA-N 0.000 claims abstract description 4
- 125000003342 alkenyl group Chemical group 0.000 claims abstract description 4
- 125000000217 alkyl group Chemical group 0.000 claims abstract description 3
- 150000007942 carboxylates Chemical class 0.000 claims abstract description 3
- MHAJPDPJQMAIIY-UHFFFAOYSA-N Hydrogen peroxide Chemical compound OO MHAJPDPJQMAIIY-UHFFFAOYSA-N 0.000 claims description 23
- 238000000034 method Methods 0.000 claims description 22
- QAHREYKOYSIQPH-UHFFFAOYSA-L cobalt(II) acetate Chemical group [Co+2].CC([O-])=O.CC([O-])=O QAHREYKOYSIQPH-UHFFFAOYSA-L 0.000 claims description 20
- 230000008569 process Effects 0.000 claims description 20
- USFZMSVCRYTOJT-UHFFFAOYSA-N Ammonium acetate Chemical compound N.CC(O)=O USFZMSVCRYTOJT-UHFFFAOYSA-N 0.000 claims description 13
- 239000005695 Ammonium acetate Substances 0.000 claims description 13
- VHUUQVKOLVNVRT-UHFFFAOYSA-N Ammonium hydroxide Chemical compound [NH4+].[OH-] VHUUQVKOLVNVRT-UHFFFAOYSA-N 0.000 claims description 13
- 235000019257 ammonium acetate Nutrition 0.000 claims description 13
- 229940043376 ammonium acetate Drugs 0.000 claims description 13
- AFVFQIVMOAPDHO-UHFFFAOYSA-M Methanesulfonate Chemical compound CS([O-])(=O)=O AFVFQIVMOAPDHO-UHFFFAOYSA-M 0.000 claims description 9
- 229910002651 NO3 Inorganic materials 0.000 claims description 8
- NHNBFGGVMKEFGY-UHFFFAOYSA-N Nitrate Chemical compound [O-][N+]([O-])=O NHNBFGGVMKEFGY-UHFFFAOYSA-N 0.000 claims description 8
- -1 fluoroborate Chemical compound 0.000 claims description 8
- 125000002496 methyl group Chemical group [H]C([H])([H])* 0.000 claims description 4
- 150000003863 ammonium salts Chemical class 0.000 claims description 3
- 150000004700 cobalt complex Chemical class 0.000 claims description 3
- 239000000908 ammonium hydroxide Substances 0.000 claims description 2
- 150000001244 carboxylic acid anhydrides Chemical class 0.000 claims description 2
- VLTRZXGMWDSKGL-UHFFFAOYSA-M perchlorate Inorganic materials [O-]Cl(=O)(=O)=O VLTRZXGMWDSKGL-UHFFFAOYSA-M 0.000 claims description 2
- VLTRZXGMWDSKGL-UHFFFAOYSA-N perchloric acid Chemical compound OCl(=O)(=O)=O VLTRZXGMWDSKGL-UHFFFAOYSA-N 0.000 claims description 2
- 150000008044 alkali metal hydroxides Chemical class 0.000 claims 1
- 230000001590 oxidative effect Effects 0.000 abstract 1
- 239000000243 solution Substances 0.000 description 88
- 238000007792 addition Methods 0.000 description 27
- KFSLWBXXFJQRDL-UHFFFAOYSA-N Peracetic acid Chemical compound CC(=O)OO KFSLWBXXFJQRDL-UHFFFAOYSA-N 0.000 description 26
- HEMHJVSKTPXQMS-UHFFFAOYSA-M Sodium hydroxide Chemical compound [OH-].[Na+] HEMHJVSKTPXQMS-UHFFFAOYSA-M 0.000 description 24
- 239000000047 product Substances 0.000 description 19
- 238000003556 assay Methods 0.000 description 17
- VWDWKYIASSYTQR-UHFFFAOYSA-N sodium nitrate Chemical compound [Na+].[O-][N+]([O-])=O VWDWKYIASSYTQR-UHFFFAOYSA-N 0.000 description 16
- WFDIJRYMOXRFFG-UHFFFAOYSA-N Acetic anhydride Chemical compound CC(=O)OC(C)=O WFDIJRYMOXRFFG-UHFFFAOYSA-N 0.000 description 15
- 238000001816 cooling Methods 0.000 description 15
- XLYOFNOQVPJJNP-UHFFFAOYSA-N water Substances O XLYOFNOQVPJJNP-UHFFFAOYSA-N 0.000 description 14
- QTBSBXVTEAMEQO-UHFFFAOYSA-N Acetic acid Chemical compound CC(O)=O QTBSBXVTEAMEQO-UHFFFAOYSA-N 0.000 description 13
- NLXLAEXVIDQMFP-UHFFFAOYSA-N Ammonium chloride Substances [NH4+].[Cl-] NLXLAEXVIDQMFP-UHFFFAOYSA-N 0.000 description 12
- 235000011114 ammonium hydroxide Nutrition 0.000 description 12
- 238000001556 precipitation Methods 0.000 description 12
- GRYLNZFGIOXLOG-UHFFFAOYSA-N Nitric acid Chemical compound O[N+]([O-])=O GRYLNZFGIOXLOG-UHFFFAOYSA-N 0.000 description 11
- 239000000463 material Substances 0.000 description 11
- 229910017604 nitric acid Inorganic materials 0.000 description 11
- GVPFVAHMJGGAJG-UHFFFAOYSA-L cobalt dichloride Chemical group [Cl-].[Cl-].[Co+2] GVPFVAHMJGGAJG-UHFFFAOYSA-L 0.000 description 10
- 238000007254 oxidation reaction Methods 0.000 description 10
- QTBSBXVTEAMEQO-UHFFFAOYSA-M Acetate Chemical compound CC([O-])=O QTBSBXVTEAMEQO-UHFFFAOYSA-M 0.000 description 9
- 238000004458 analytical method Methods 0.000 description 9
- 230000003647 oxidation Effects 0.000 description 9
- 239000007858 starting material Substances 0.000 description 9
- 229940011182 cobalt acetate Drugs 0.000 description 8
- 238000002474 experimental method Methods 0.000 description 8
- 101150100654 pacC gene Proteins 0.000 description 8
- 238000002360 preparation method Methods 0.000 description 8
- 235000011121 sodium hydroxide Nutrition 0.000 description 8
- 239000004317 sodium nitrate Substances 0.000 description 8
- 235000010344 sodium nitrate Nutrition 0.000 description 8
- VEXZGXHMUGYJMC-UHFFFAOYSA-N Hydrochloric acid Chemical compound Cl VEXZGXHMUGYJMC-UHFFFAOYSA-N 0.000 description 7
- 239000002002 slurry Substances 0.000 description 7
- VEXZGXHMUGYJMC-UHFFFAOYSA-M Chloride anion Chemical compound [Cl-] VEXZGXHMUGYJMC-UHFFFAOYSA-M 0.000 description 6
- OKKJLVBELUTLKV-UHFFFAOYSA-N Methanol Chemical compound OC OKKJLVBELUTLKV-UHFFFAOYSA-N 0.000 description 6
- 239000002253 acid Substances 0.000 description 6
- 239000000872 buffer Substances 0.000 description 6
- 239000007787 solid Substances 0.000 description 6
- 238000003756 stirring Methods 0.000 description 6
- 150000008064 anhydrides Chemical class 0.000 description 5
- 239000000460 chlorine Substances 0.000 description 5
- 229940097267 cobaltous chloride Drugs 0.000 description 5
- 229910000069 nitrogen hydride Inorganic materials 0.000 description 5
- 150000002978 peroxides Chemical class 0.000 description 5
- QVGXLLKOCUKJST-UHFFFAOYSA-N atomic oxygen Chemical compound [O] QVGXLLKOCUKJST-UHFFFAOYSA-N 0.000 description 4
- 239000001301 oxygen Substances 0.000 description 4
- 229910052760 oxygen Inorganic materials 0.000 description 4
- 239000002244 precipitate Substances 0.000 description 4
- 150000003839 salts Chemical class 0.000 description 4
- 239000006228 supernatant Substances 0.000 description 4
- KZBUYRJDOAKODT-UHFFFAOYSA-N Chlorine Chemical compound ClCl KZBUYRJDOAKODT-UHFFFAOYSA-N 0.000 description 3
- KWYUFKZDYYNOTN-UHFFFAOYSA-M Potassium hydroxide Chemical compound [OH-].[K+] KWYUFKZDYYNOTN-UHFFFAOYSA-M 0.000 description 3
- 239000000203 mixture Substances 0.000 description 3
- 125000002924 primary amino group Chemical group [H]N([H])* 0.000 description 3
- 238000011084 recovery Methods 0.000 description 3
- 238000005406 washing Methods 0.000 description 3
- HZAXFHJVJLSVMW-UHFFFAOYSA-N 2-Aminoethan-1-ol Chemical compound NCCO HZAXFHJVJLSVMW-UHFFFAOYSA-N 0.000 description 2
- ZAMOUSCENKQFHK-UHFFFAOYSA-N Chlorine atom Chemical compound [Cl] ZAMOUSCENKQFHK-UHFFFAOYSA-N 0.000 description 2
- QUSNBJAOOMFDIB-UHFFFAOYSA-N Ethylamine Chemical compound CCN QUSNBJAOOMFDIB-UHFFFAOYSA-N 0.000 description 2
- AFVFQIVMOAPDHO-UHFFFAOYSA-N Methanesulfonic acid Chemical compound CS(O)(=O)=O AFVFQIVMOAPDHO-UHFFFAOYSA-N 0.000 description 2
- BAVYZALUXZFZLV-UHFFFAOYSA-N Methylamine Chemical compound NC BAVYZALUXZFZLV-UHFFFAOYSA-N 0.000 description 2
- FAPWRFPIFSIZLT-UHFFFAOYSA-M Sodium chloride Chemical compound [Na+].[Cl-] FAPWRFPIFSIZLT-UHFFFAOYSA-M 0.000 description 2
- QAOWNCQODCNURD-UHFFFAOYSA-L Sulfate Chemical compound [O-]S([O-])(=O)=O QAOWNCQODCNURD-UHFFFAOYSA-L 0.000 description 2
- 239000007864 aqueous solution Substances 0.000 description 2
- 150000004982 aromatic amines Chemical class 0.000 description 2
- 230000008901 benefit Effects 0.000 description 2
- 230000003139 buffering effect Effects 0.000 description 2
- 229910052801 chlorine Inorganic materials 0.000 description 2
- 229910000001 cobalt(II) carbonate Inorganic materials 0.000 description 2
- 150000001875 compounds Chemical class 0.000 description 2
- 239000013078 crystal Substances 0.000 description 2
- PAFZNILMFXTMIY-UHFFFAOYSA-N cyclohexylamine Chemical compound NC1CCCCC1 PAFZNILMFXTMIY-UHFFFAOYSA-N 0.000 description 2
- 239000011521 glass Substances 0.000 description 2
- 238000004128 high performance liquid chromatography Methods 0.000 description 2
- 230000007062 hydrolysis Effects 0.000 description 2
- 238000006460 hydrolysis reaction Methods 0.000 description 2
- 239000004570 mortar (masonry) Substances 0.000 description 2
- 150000002823 nitrates Chemical class 0.000 description 2
- 150000002891 organic anions Chemical class 0.000 description 2
- UPWOEMHINGJHOB-UHFFFAOYSA-N oxo(oxocobaltiooxy)cobalt Chemical compound O=[Co]O[Co]=O UPWOEMHINGJHOB-UHFFFAOYSA-N 0.000 description 2
- 229910021653 sulphate ion Inorganic materials 0.000 description 2
- PAWQVTBBRAZDMG-UHFFFAOYSA-N 2-(3-bromo-2-fluorophenyl)acetic acid Chemical compound OC(=O)CC1=CC=CC(Br)=C1F PAWQVTBBRAZDMG-UHFFFAOYSA-N 0.000 description 1
- MCSXGCZMEPXKIW-UHFFFAOYSA-N 3-hydroxy-4-[(4-methyl-2-nitrophenyl)diazenyl]-N-(3-nitrophenyl)naphthalene-2-carboxamide Chemical compound Cc1ccc(N=Nc2c(O)c(cc3ccccc23)C(=O)Nc2cccc(c2)[N+]([O-])=O)c(c1)[N+]([O-])=O MCSXGCZMEPXKIW-UHFFFAOYSA-N 0.000 description 1
- QGZKDVFQNNGYKY-UHFFFAOYSA-O Ammonium Chemical compound [NH4+] QGZKDVFQNNGYKY-UHFFFAOYSA-O 0.000 description 1
- PAYRUJLWNCNPSJ-UHFFFAOYSA-N Aniline Chemical compound NC1=CC=CC=C1 PAYRUJLWNCNPSJ-UHFFFAOYSA-N 0.000 description 1
- BVKZGUZCCUSVTD-UHFFFAOYSA-L Carbonate Chemical compound [O-]C([O-])=O BVKZGUZCCUSVTD-UHFFFAOYSA-L 0.000 description 1
- 229910021580 Cobalt(II) chloride Inorganic materials 0.000 description 1
- PIICEJLVQHRZGT-UHFFFAOYSA-N Ethylenediamine Chemical compound NCCN PIICEJLVQHRZGT-UHFFFAOYSA-N 0.000 description 1
- VZCYOOQTPOCHFL-OWOJBTEDSA-N Fumaric acid Chemical compound OC(=O)\C=C\C(O)=O VZCYOOQTPOCHFL-OWOJBTEDSA-N 0.000 description 1
- WHUUTDBJXJRKMK-VKHMYHEASA-N L-glutamic acid Chemical compound OC(=O)[C@@H](N)CCC(O)=O WHUUTDBJXJRKMK-VKHMYHEASA-N 0.000 description 1
- OFOBLEOULBTSOW-UHFFFAOYSA-L Malonate Chemical compound [O-]C(=O)CC([O-])=O OFOBLEOULBTSOW-UHFFFAOYSA-L 0.000 description 1
- 229910019142 PO4 Inorganic materials 0.000 description 1
- VMHLLURERBWHNL-UHFFFAOYSA-M Sodium acetate Chemical compound [Na+].CC([O-])=O VMHLLURERBWHNL-UHFFFAOYSA-M 0.000 description 1
- 230000002378 acidificating effect Effects 0.000 description 1
- 150000007513 acids Chemical class 0.000 description 1
- 230000004913 activation Effects 0.000 description 1
- 125000001931 aliphatic group Chemical group 0.000 description 1
- 239000003513 alkali Substances 0.000 description 1
- 229910001963 alkali metal nitrate Inorganic materials 0.000 description 1
- 150000003973 alkyl amines Chemical class 0.000 description 1
- 125000003277 amino group Chemical group 0.000 description 1
- 235000019270 ammonium chloride Nutrition 0.000 description 1
- 239000012736 aqueous medium Substances 0.000 description 1
- 239000002585 base Substances 0.000 description 1
- 230000009286 beneficial effect Effects 0.000 description 1
- 238000004061 bleaching Methods 0.000 description 1
- 230000021523 carboxylation Effects 0.000 description 1
- 238000006473 carboxylation reaction Methods 0.000 description 1
- 125000002579 carboxylato group Chemical group [O-]C(*)=O 0.000 description 1
- 150000001732 carboxylic acid derivatives Chemical class 0.000 description 1
- 230000015556 catabolic process Effects 0.000 description 1
- 230000008859 change Effects 0.000 description 1
- 239000003795 chemical substances by application Substances 0.000 description 1
- ZBYYWKJVSFHYJL-UHFFFAOYSA-L cobalt(2+);diacetate;tetrahydrate Chemical compound O.O.O.O.[Co+2].CC([O-])=O.CC([O-])=O ZBYYWKJVSFHYJL-UHFFFAOYSA-L 0.000 description 1
- 239000002131 composite material Substances 0.000 description 1
- 238000000354 decomposition reaction Methods 0.000 description 1
- 238000006731 degradation reaction Methods 0.000 description 1
- 150000004985 diamines Chemical class 0.000 description 1
- 230000003292 diminished effect Effects 0.000 description 1
- 230000000694 effects Effects 0.000 description 1
- 230000007613 environmental effect Effects 0.000 description 1
- 238000001704 evaporation Methods 0.000 description 1
- 230000008020 evaporation Effects 0.000 description 1
- 238000001914 filtration Methods 0.000 description 1
- 229930195712 glutamate Natural products 0.000 description 1
- 231100001261 hazardous Toxicity 0.000 description 1
- 238000010438 heat treatment Methods 0.000 description 1
- 150000004678 hydrides Chemical class 0.000 description 1
- 125000004435 hydrogen atom Chemical group [H]* 0.000 description 1
- XLYOFNOQVPJJNP-UHFFFAOYSA-M hydroxide Chemical compound [OH-] XLYOFNOQVPJJNP-UHFFFAOYSA-M 0.000 description 1
- 239000005457 ice water Substances 0.000 description 1
- 230000006872 improvement Effects 0.000 description 1
- 239000012535 impurity Substances 0.000 description 1
- 238000011065 in-situ storage Methods 0.000 description 1
- ICIWUVCWSCSTAQ-UHFFFAOYSA-N iodic acid Chemical class OI(=O)=O ICIWUVCWSCSTAQ-UHFFFAOYSA-N 0.000 description 1
- 238000002955 isolation Methods 0.000 description 1
- 239000007788 liquid Substances 0.000 description 1
- 239000007800 oxidant agent Substances 0.000 description 1
- ZRZYLFPZOSSVFG-UHFFFAOYSA-N pentaazanium;pentaacetate Chemical compound [NH4+].[NH4+].[NH4+].[NH4+].[NH4+].CC([O-])=O.CC([O-])=O.CC([O-])=O.CC([O-])=O.CC([O-])=O ZRZYLFPZOSSVFG-UHFFFAOYSA-N 0.000 description 1
- NIXKBAZVOQAHGC-UHFFFAOYSA-N phenylmethanesulfonic acid Chemical compound OS(=O)(=O)CC1=CC=CC=C1 NIXKBAZVOQAHGC-UHFFFAOYSA-N 0.000 description 1
- 235000021317 phosphate Nutrition 0.000 description 1
- 150000003013 phosphoric acid derivatives Chemical class 0.000 description 1
- 229920000768 polyamine Polymers 0.000 description 1
- 238000012545 processing Methods 0.000 description 1
- WYVAMUWZEOHJOQ-UHFFFAOYSA-N propionic anhydride Chemical compound CCC(=O)OC(=O)CC WYVAMUWZEOHJOQ-UHFFFAOYSA-N 0.000 description 1
- 239000002994 raw material Substances 0.000 description 1
- 239000000376 reactant Substances 0.000 description 1
- 239000011541 reaction mixture Substances 0.000 description 1
- 238000007086 side reaction Methods 0.000 description 1
- 239000001632 sodium acetate Substances 0.000 description 1
- 235000017281 sodium acetate Nutrition 0.000 description 1
- 239000011780 sodium chloride Substances 0.000 description 1
- KDYFGRWQOYBRFD-UHFFFAOYSA-L succinate(2-) Chemical compound [O-]C(=O)CCC([O-])=O KDYFGRWQOYBRFD-UHFFFAOYSA-L 0.000 description 1
- 238000012360 testing method Methods 0.000 description 1
- VZCYOOQTPOCHFL-UHFFFAOYSA-N trans-butenedioic acid Natural products OC(=O)C=CC(O)=O VZCYOOQTPOCHFL-UHFFFAOYSA-N 0.000 description 1
- 238000012546 transfer Methods 0.000 description 1
- 239000002699 waste material Substances 0.000 description 1
Classifications
-
- C—CHEMISTRY; METALLURGY
- C07—ORGANIC CHEMISTRY
- C07F—ACYCLIC, CARBOCYCLIC OR HETEROCYCLIC COMPOUNDS CONTAINING ELEMENTS OTHER THAN CARBON, HYDROGEN, HALOGEN, OXYGEN, NITROGEN, SULFUR, SELENIUM OR TELLURIUM
- C07F15/00—Compounds containing elements of Groups 8, 9, 10 or 18 of the Periodic Table
- C07F15/06—Cobalt compounds
- C07F15/065—Cobalt compounds without a metal-carbon linkage
-
- B—PERFORMING OPERATIONS; TRANSPORTING
- B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
- B01J—CHEMICAL OR PHYSICAL PROCESSES, e.g. CATALYSIS OR COLLOID CHEMISTRY; THEIR RELEVANT APPARATUS
- B01J31/00—Catalysts comprising hydrides, coordination complexes or organic compounds
- B01J31/16—Catalysts comprising hydrides, coordination complexes or organic compounds containing coordination complexes
- B01J31/18—Catalysts comprising hydrides, coordination complexes or organic compounds containing coordination complexes containing nitrogen, phosphorus, arsenic or antimony as complexing atoms, e.g. in pyridine ligands, or in resonance therewith, e.g. in isocyanide ligands C=N-R or as complexed central atoms
- B01J31/1805—Catalysts comprising hydrides, coordination complexes or organic compounds containing coordination complexes containing nitrogen, phosphorus, arsenic or antimony as complexing atoms, e.g. in pyridine ligands, or in resonance therewith, e.g. in isocyanide ligands C=N-R or as complexed central atoms the ligands containing nitrogen
-
- B—PERFORMING OPERATIONS; TRANSPORTING
- B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
- B01J—CHEMICAL OR PHYSICAL PROCESSES, e.g. CATALYSIS OR COLLOID CHEMISTRY; THEIR RELEVANT APPARATUS
- B01J31/00—Catalysts comprising hydrides, coordination complexes or organic compounds
- B01J31/16—Catalysts comprising hydrides, coordination complexes or organic compounds containing coordination complexes
- B01J31/22—Organic complexes
- B01J31/2204—Organic complexes the ligands containing oxygen or sulfur as complexing atoms
- B01J31/2208—Oxygen, e.g. acetylacetonates
- B01J31/2226—Anionic ligands, i.e. the overall ligand carries at least one formal negative charge
-
- B—PERFORMING OPERATIONS; TRANSPORTING
- B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
- B01J—CHEMICAL OR PHYSICAL PROCESSES, e.g. CATALYSIS OR COLLOID CHEMISTRY; THEIR RELEVANT APPARATUS
- B01J2231/00—Catalytic reactions performed with catalysts classified in B01J31/00
- B01J2231/70—Oxidation reactions, e.g. epoxidation, (di)hydroxylation, dehydrogenation and analogues
-
- B—PERFORMING OPERATIONS; TRANSPORTING
- B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
- B01J—CHEMICAL OR PHYSICAL PROCESSES, e.g. CATALYSIS OR COLLOID CHEMISTRY; THEIR RELEVANT APPARATUS
- B01J2531/00—Additional information regarding catalytic systems classified in B01J31/00
- B01J2531/80—Complexes comprising metals of Group VIII as the central metal
- B01J2531/84—Metals of the iron group
- B01J2531/845—Cobalt
Definitions
- This invention relates to a process for the preparation of cobalt complexes and to cobalt complexes obtained thereby.
- Co III complexes of Co III act as oxidation catalysts and therefore promote reaction of various oxygen species. These reactions generally occur in water or an aqueous medium.
- cobalt complexes are useful as oxidation catalysts or promoters of oxidation reactions with atmospheric oxygen or oxygen transfer agents such as peroxides, per iodates and amine oxides.
- a particular use of trivalent cobalt complexes is as bleaching catalysts for the activation of, for example, perborates.
- the cobalt complexes originally proposed possessed an inner chloride anion but these have been found to be to prone to hydrolysis such that the complexes with an acetate inner anion are more useful. These acetato cobalt complexes are preferred for reactions in water since they give rise to less side reactions. This is because there is less hydrolysis or degradation of the catalyst and also less precipitation of such products which can give rise to fouling etc.
- a typical acetato cobalt complex has the formula Co(NH 3 ) 3 !Cl 2 (hereafter referred to a PAAC).
- the starting material for the preparation of such a complex is cobalt chloride which has the formula Co II (H 2 O) 6 !Cl 2 .
- Reaction with ammonia or an amine gives rise to the corresponding amino complex which, an oxidation, produces the compound of the formula Co III (NH 3 ) 5 H 2 O!Cl 3 (hereafter referred to as PAQC) together with Co III (NH 3 ) 6 !Cl 3 (HAC).
- PAQC Co III
- HAC Co III
- Reaction of PAQC with hot hydrochloric add gives rise to Co III (NH 3 ) 5 !Cl!Cl 2 (PACC).
- each R which may be the same or different, represents hydrogen or an optionally substituted hydrocarbon group and R 1 represents an alkyl or alkenyl group of 1 to 18, especially 1 to 6, carbon atoms, preferably methyl, at a pH above 8.5; and optionally
- a typical starting material is cobaltous chloride.
- This has the disadvantage that in the strongly oxidising conditions used to produce cobalt (III) oxide, the chloride counter ions may react to form potentially hazardous chlorine. Accordingly it is preferable to use cobaltous acetate as the starting material.
- Other starting materials include the oxide and hydroxide. It will be appreciated that the nature of the anion in the starting material is significant. Thus the use of cobaltous chloride will tend to give rise to the production of some PACC.
- the complex typically is an ammonium complex i.e. one in which R represents hydrogen.
- corresponding amino complexes can be obtained by reaction with amines having for example, 1 to 8, especially 1 to 6, carbon atoms, including alkyl amines such as methylamine and ethylamine, aromatic amines such as phenylamine, and cyclic amines such as cyclohexylamine as well as hydroxy amines such as ethanolamine as well as polyamines, typically diamines, such as ethylenediamine.
- R can represent a hydrocarbon group which may itself be substituted by an amino group in which case the number of R groups present will be reduced below 5 in order to balance the molecule.
- the expression "amine” will be used herein to denote ammonia as well as aliphatic and aromatic amines.
- an aqueous ammonia (or amine) solution is used to react with an aqueous solution of the cobalt salt.
- This reaction should be allowed to proceed slowly since it is significantly exothermic.
- an ammonium salt typically ammonium acetate, is also used; this reduces the pH to, say, 8 to 9 as opposed to 10 or more and enhances oxidation. Consequently the use of such a salt can reduce the mount of oxidising agent necessary in the subsequent step.
- the use of all liquid raw materials simplifies production. As indicated above, a maximum of 15 molar equivalents of amine species should be used.
- aqueous solution generally having a pH from 8 to 10 and preferably from 9 to 10.
- the amine complex is then oxidised. This is typically performed using hydrogen peroxide although aerial oxidation is also a possibility. 0.5 moles of hydrogen peroxide are required for stoichiometric purposes but, in practice, an excess of hydrogen peroxide is desirable. It has been found, though, that a large excess of hydrogen peroxide such as 2 moles is generally undesirable. This is because of the potential problem that the counter chloride ions present when cobaltous chloride is used as the starting material may be oxidised to chlorine causing a safety hazard. Thus the amount employed is typically from 0.5 to 1 moles.
- conversion step (iii) is carried out with the corresponding carboxylic acid an hydride of formula (R 1 CO) 2 O.
- step (ii) it has been found desirable to raise the pH of the solution resulting from step (ii), typically at a temperature from 50° C. to 80° C., especially 60° to 65° C., by the addition of an alkali such as sodium hydroxide or, for example, potassium hydroxide.
- an alkali such as sodium hydroxide or, for example, potassium hydroxide.
- Ammonium hydroxide is generally less desirable to use.
- This pH is suitably raised from 7 to 8.5 to, say, 9 to 12, preferably 10 to 11.5. It is believed that when the starting material is cobaltous chloride, this addition causes PACC to be converted to PAQC which can more readily be carboxylated.
- step (i) the increased pH due to ammonia addition is neutralised to enhance oxidation by a mildly acidic material while before carboxylation the pH is increased.
- This solution is then desirably cooled, for example to room temperature (20°-25° C.) and then the carboxylic acid anhydride is added.
- carboxylic acid anhydride is added.
- acetic anhydride is used for this purpose although peracetic acid and acetic acid can also be used. It should be added slowly since the reaction is significantly exothermic and it is desirable to cool the reaction vessel, for example to keep the temperature from exceeding, say, 40° C.
- step (iii) can be obtained with very little impurities.
- cobaltous chloride is used as the starting material, little or no PACC is present.
- This product generally does not precipitate because of its very high solubility and can be isolated by evaporation.
- step (iii) is performed by increasing the amount of ammonium carboxylate added to the initial reaction mixture.
- the cobalt (II) salt is Co(R 1 COO) 2 , especially Where R 1 is methyl, or where the molar ratio of the ammonium carboxylate to the cobalt salt is from 3:1 to 4:1 and/or where the molar ratio of ammonia to the cobalt salt is from 4:1 to 7:1, particularly from 5:1 to 6:1.
- An advantage of the preferred embodiment of the invention is it does not involve the use of strong bases which have to be used with care because of the danger of decomposition.
- a further advantage is that the concentration of ammonia used is even less, reducing waste because there is less ammonia to distil off at the end of step (ii) and reducing the amount of washing required to remove the hexa ammonia complex (HAC) because less of this complex is formed.
- the X anion can be replaced by a different anion by a metathetical reaction in order that a new salt which is less soluble is obtained which may precipitate.
- a new salt which is less soluble is obtained which may precipitate.
- the conversion of the counter ion is carried out before the reaction solution is allowed to cool. This is advantageous because larger crystal sizes are produced in the precipitate which are easier to filter.
- Counter ions can be used for this purpose, of which the most preferred are the nitrate, fluoroborate and methane sulphonate (PAAN, PAAFB and PAAMS for the acetato complex) along with the perchlorate.
- Other anions which may be used include the sulphate, carbonate and various phosphates along with a variety of organic anions including the acetate, glutamate, succinate, malonate, fumarate and toluene sulphonate.
- Typical organic anions include those of the formula R 2 COO where R 2 represents an optionally hydroxy substituted alkyl or alkenyl group 1 to 18, for example 1 to 6, carbon atoms.
- nitric acid or a suitable nitrate salt e.g. an alkali metal nitrate
- the molar ratio of nitric acid or nitrate salt to cobalt(II) starting material is from 2:1 to 5:1, more preferably 2:1 to 3:1.
- the ammonia solution at 25° C. and ammonium acetate were charged to a stirred 31 RB Quickfit flask equipped with a condenser and reaction temperature-controller; after stirring 5 minutes the resulting solution registered 5° C.
- the cobalt chloride solution was added over 15 minutes in a steady stream resulting in an exotherm to 41° C. after approximately 3/4 of the addition; at the end of the addition the temperature in the flask was 38° C. After stirring 40 minutes the red solution was at 33° C. and registered pH 8.66; a trace of solid was observed in the flask.
- the hydrogen peroxide solution was added over 50 minutes during which time the temperature in the flask rose to 56° C.
- each drop produced a vigorous effervescence upon contact with the flask contents; towards the end the effervescence at the point of contact diminished significantly being replaced by a gentle effervescence across the surface and the solution developed a more intense red colour.
- the mantle was set to heat to 65° C.; at 60° C. the solution registered pH 7.9 and the caustic soda addition was started; it lasted 15 minutes during which time an exotherm was observed and the temperature peaked at 70° C. After stirring a further 30 minutes the temperature had dropped back to 65° C. and the solution registered pH 10.6 having peaked at 11.1; no solid was observed in the flask. After cooling to 27° C. the solution registered pH 11.2.
- the wet-cake was dried in a fan over at 80° C. for 2 hours, and ground in a mortar and pestle before analysis;
- the liquor registered pH 3.6. It was analyzed by HPLC and found to contain product equivalent to 20 g PAAN, i.e. 5% of Co charge.
- the nitric acid charge equates to 2 mole equivalents to Co, i.e. 2/3 the amount used in Example 1.
- the liquor has a brown-black colour; it darkens during the nitric acid addition. It has a strong odor of acetic acid and the following approximate composition calculated by difference from the charges and dried product, assuming for the time being that "non-PAA cobalt" is present as HAC complex;
- the complexes contain 10 g cobalt i.e. 0.43% Wt. in the liquor.
- Example 2 There were no significant differences to Example 2 up to the end of the anhydride addition when the flask contained 2461 g solution with pH 4.8 and an assay of 14.9% PAAC i.e. 89% conversion from Cobalt.
- the slurry was filtered through two No1 porosity sintered-glass Buchner funnels under vacuum, the cake was washed with a total of 600 mls methanol and left in the funnel overnight then dried for an hour in a fan oven at 80° C., and ground in a mortar and pestle before analysis.
- a batch of solution was prepared as for PAAMS (Example 3) with c. 3.5 hours for the anhydride addition.
- the yield was 2481 g with pH 4.83 and assay 14.6% PAAC, i.e. 88% conversion.
- the desired product was made by sodium fluoroborate precipitation and water washing from a composite sample of "PAA" solutions prepared in the presence of chloride and acetate ions, i.e. samples from both cobalt salts+"opposite” buffering add.
- the "PAA” solution assayed 13.0% as PAAC and contained practically no PACC.
- Cobalt acetate was quickly added to freshly prepared ammonia buffer at 11° C. to form a clear solution at a temperature of 26° C.
- the hydrogen peroxide solution was then added over 20 minutes without cooling during which time the temperature of the solution rose from 26° C. to 49° C.
- the solution was then stirred for one hour. After stirring, the temperature of the solution was 33° C. It was then heated to a temperature of 80° C. It was then maintained at this temperature for six hours.
- the sodium nitrate solution was added over a period of 20 minutes. 20 minutes after the addition of the sodium nitrate solution, the solution was cooled and after an hour, it was filtered and washed with iced water. The product filtered slowly and gave a very wet cake (approximately 30% water) which was dried in an oven at 70° C.
- Cobalt acetate was added quickly to freshly prepared ammonia buffer without cooling.
- the resultant solution was dear and had a temperature of 23° C. Air was then bubbled through the solution at a rate of 800 ml/min and was left on overnight. After approximately 20 hours, the air supply was stopped and the solution was heated to 80° C. and this temperature was maintained for six hours. At the end of the heating, the solution was cooled.
- Cobalt acetate was added to freshly prepared ammonia buffer quickly without cooling.
- the resultant solution was clear and had a temperature of 28° C.
- Peroxide solution was then added over a period of 50 minutes without cooling.
- the resultant solution which had a temperature of 59° C. was then stirred for 40 minutes.
- the stirred solution was heated to 80° C. and this temperature was maintained for six hours. The solution was then cooled.
- Cobalt acetate was added to freshly prepared ammonia buffer quickly without cooling.
- the resultant solution had a temperature of 26° C. and after 60 minutes, the hydrogen peroxide solution was added over a period of 33/4 hours. Frothing was observed towards the end of the peroxide addition and water was used to wash down the condenser. After the addition of peroxide, the solution was maintained at a temperature of 46° C. for 20 minutes. It was then heated to 80° C. and maintained over night before being cooled.
- the conversion rate of cobalt based on the PAAA assay was 86.4%.
- Cobalt acetate was added to freshly prepared ammonia buffer quickly without cooling.
- the resultant solution was clear and had a temperature of 27° C.
- air was bubbled through the solution at a rate of 1800 ml/min and the air was left on overnight. Approximately 20 hours later, the air supply was stopped and the solution was heated to 80° C. and maintained at this temperature for 6 hours before being cooled.
- the mass balance showed that 32 g was lost per mole of cobalt in the experiment.
- the conversion rate of cobalt based on the PAAA assay was 70.0%.
- the first aliquot of sodium nitrate was added over a period of 55 minutes without cooling. Precipitation started with the first few drops and was mildly exothermic. The final temperature of the solution was 30° C. and an assay of the supernatant after addition of the first aliquot showed that less than 5% of PAA remained in the solution.
- the second aliquot of sodium nitrate was then added after a wait of 35 minutes over a period of 15 minutes. An assay of the supernatant after the addition of the second aliquot showed that an insignificant mount of PAA remained in the solution. After one hour, the precipitate was filtered and washed with 200 ml of ice water.
- the first aliquot of nitric acid was added over a period of 20 minutes without cooling. Precipitation started with the first few drops and was highly exothermic. The final temperature was 59° C. An assay of the supernatant after the addition of the first aliquot showed that less than 5% of PAA remained in the solution. Cooling was then applied for 1/2 hour until a temperature of 18° C. was reached and then the second aliquot was added over a period of 10 minutes. An assay of the supernatant after the addition of the second aliquot showed that an insignificant trace of PAA remained in the solution. The product was cooled for 40 minutes then filtered and washed with 240 ml iced water.
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Abstract
A process for preparing a cobalt (III) complex is described which comprises: (i) treating a divalent cobalt salt of formula CoII X2/n where n is the valency of an anion X, with up to 15 molar equivalents of ammonia or an amine; (ii) oxidizing the resulting amine complex; (iii) converting the oxidized complex to the corresponding carboxylate of formula CoIII (NR3)5 R1 COO!X2/n where each R, which may be the same or different, represents hydrogen or an optionally substituted hydrocarbon group and R1 represents an alkyl or alkenyl group of 1 to 18 carbon atoms, at a pH above 8.5; and optionally (iv) replacing the X ion by a different anion by a metathetical reaction.
Description
This application was filed under 35 U.S.C. 371 as a request for U.S. examination of International application No. PCT/GB96/01986, filed on Aug. 14, 1996.
This invention relates to a process for the preparation of cobalt complexes and to cobalt complexes obtained thereby.
Complexes of CoIII act as oxidation catalysts and therefore promote reaction of various oxygen species. These reactions generally occur in water or an aqueous medium. Thus cobalt complexes are useful as oxidation catalysts or promoters of oxidation reactions with atmospheric oxygen or oxygen transfer agents such as peroxides, per iodates and amine oxides. A particular use of trivalent cobalt complexes is as bleaching catalysts for the activation of, for example, perborates.
The cobalt complexes originally proposed possessed an inner chloride anion but these have been found to be to prone to hydrolysis such that the complexes with an acetate inner anion are more useful. These acetato cobalt complexes are preferred for reactions in water since they give rise to less side reactions. This is because there is less hydrolysis or degradation of the catalyst and also less precipitation of such products which can give rise to fouling etc.
A typical acetato cobalt complex has the formula Co(NH3)3 !Cl2 (hereafter referred to a PAAC). The starting material for the preparation of such a complex is cobalt chloride which has the formula CoII (H2 O)6 !Cl2. Reaction with ammonia or an amine gives rise to the corresponding amino complex which, an oxidation, produces the compound of the formula CoIII (NH3)5 H2 O!Cl3 (hereafter referred to as PAQC) together with CoIII (NH3)6 !Cl3 (HAC). Reaction of PAQC with hot hydrochloric add gives rise to CoIII (NH3)5 !Cl!Cl2 (PACC). This PACC can be converted into the desired PAAC although very dilute solutions have to be used, which are clearly unrealistic on an industrial scale. Clearly it would be much better if a process could be found whereby cobalt chloride is converted into the desired acetato cobalt complex without the need to prepare PACC as an intermediate. Previous attempts at this have, though, been found to be unsatisfactory and have produced the desired compound in only very small yield. A way has now been found, according to the present invention, whereby such complexes can be prepared in good yield by controlling the amount of ammonia or amine. It has been found that control of the amount of ammonia or amine employed has a significant effect on the percent conversion to the desired PAAC.
According to the present invention, there is provided a process for preparing a cobalt II complex which comprises:
(i) treating a divalent cobalt salt of formula CoII X2/n where n is the valency of an anion X, with up to 15 molar equivalents of ammonia or an amine;
(ii) oxidising the resulting amine complex;
(iii) converting the oxidised complex to the corresponding carboxylate of formula CoIII NR3)5 R1 COO!X2/n where each R, which may be the same or different, represents hydrogen or an optionally substituted hydrocarbon group and R1 represents an alkyl or alkenyl group of 1 to 18, especially 1 to 6, carbon atoms, preferably methyl, at a pH above 8.5; and optionally
(iv) replacing the X ion by a different anion by a metathetical reaction.
As indicated above, a typical starting material is cobaltous chloride. This has the disadvantage that in the strongly oxidising conditions used to produce cobalt (III) oxide, the chloride counter ions may react to form potentially hazardous chlorine. Accordingly it is preferable to use cobaltous acetate as the starting material. Other starting materials include the oxide and hydroxide. It will be appreciated that the nature of the anion in the starting material is significant. Thus the use of cobaltous chloride will tend to give rise to the production of some PACC. The complex typically is an ammonium complex i.e. one in which R represents hydrogen. This is obtained by using ammonia but it will be appreciated that corresponding amino complexes can be obtained by reaction with amines having for example, 1 to 8, especially 1 to 6, carbon atoms, including alkyl amines such as methylamine and ethylamine, aromatic amines such as phenylamine, and cyclic amines such as cyclohexylamine as well as hydroxy amines such as ethanolamine as well as polyamines, typically diamines, such as ethylenediamine. Thus R can represent a hydrocarbon group which may itself be substituted by an amino group in which case the number of R groups present will be reduced below 5 in order to balance the molecule. For simplicity, the expression "amine" will be used herein to denote ammonia as well as aliphatic and aromatic amines.
In the step (i) of the process, typically an aqueous ammonia (or amine) solution is used to react with an aqueous solution of the cobalt salt. This reaction should be allowed to proceed slowly since it is significantly exothermic. Desirably an ammonium salt, typically ammonium acetate, is also used; this reduces the pH to, say, 8 to 9 as opposed to 10 or more and enhances oxidation. Consequently the use of such a salt can reduce the mount of oxidising agent necessary in the subsequent step. Clearly the use of all liquid raw materials simplifies production. As indicated above, a maximum of 15 molar equivalents of amine species should be used. It has been found that, in general, the best results are obliged by using smaller concentrations of ammonia, typically from no more than 10 molar equivalents and, more particularly, no more than 8 molar equivalents. The resulting amine complex will be produced in aqueous solution generally having a pH from 8 to 10 and preferably from 9 to 10.
The amine complex is then oxidised. This is typically performed using hydrogen peroxide although aerial oxidation is also a possibility. 0.5 moles of hydrogen peroxide are required for stoichiometric purposes but, in practice, an excess of hydrogen peroxide is desirable. It has been found, though, that a large excess of hydrogen peroxide such as 2 moles is generally undesirable. This is because of the potential problem that the counter chloride ions present when cobaltous chloride is used as the starting material may be oxidised to chlorine causing a safety hazard. Thus the amount employed is typically from 0.5 to 1 moles.
According to one embodiment of the invention, conversion step (iii) is carried out with the corresponding carboxylic acid an hydride of formula (R1 CO)2 O.
Before this step is carried out, it has been found desirable to raise the pH of the solution resulting from step (ii), typically at a temperature from 50° C. to 80° C., especially 60° to 65° C., by the addition of an alkali such as sodium hydroxide or, for example, potassium hydroxide. Ammonium hydroxide is generally less desirable to use. This pH is suitably raised from 7 to 8.5 to, say, 9 to 12, preferably 10 to 11.5. It is believed that when the starting material is cobaltous chloride, this addition causes PACC to be converted to PAQC which can more readily be carboxylated. Thus in this preferred embodiment, in step (i) the increased pH due to ammonia addition is neutralised to enhance oxidation by a mildly acidic material while before carboxylation the pH is increased.
This solution is then desirably cooled, for example to room temperature (20°-25° C.) and then the carboxylic acid anhydride is added. Typically acetic anhydride is used for this purpose although peracetic acid and acetic acid can also be used. It should be added slowly since the reaction is significantly exothermic and it is desirable to cool the reaction vessel, for example to keep the temperature from exceeding, say, 40° C.
A particular feature of the process for the present invention is that the product of step (iii) can be obtained with very little impurities. In particular where cobaltous chloride is used as the starting material, little or no PACC is present. This product generally does not precipitate because of its very high solubility and can be isolated by evaporation.
According to a preferred embodiment of the invention, step (iii) is performed by increasing the amount of ammonium carboxylate added to the initial reaction mixture. Particularly good results are obtained by this method when the cobalt (II) salt is Co(R1 COO)2, especially Where R1 is methyl, or where the molar ratio of the ammonium carboxylate to the cobalt salt is from 3:1 to 4:1 and/or where the molar ratio of ammonia to the cobalt salt is from 4:1 to 7:1, particularly from 5:1 to 6:1.
An advantage of the preferred embodiment of the invention is it does not involve the use of strong bases which have to be used with care because of the danger of decomposition.
A further advantage is that the concentration of ammonia used is even less, reducing waste because there is less ammonia to distil off at the end of step (ii) and reducing the amount of washing required to remove the hexa ammonia complex (HAC) because less of this complex is formed.
According to another feature of the present invention, the X anion can be replaced by a different anion by a metathetical reaction in order that a new salt which is less soluble is obtained which may precipitate. In other words by replacing the chloride ion by a different "counter ion" which gives rise to a much less soluble complex it is possible to isolate the complex much more simply, for example by precipitation. Preferably the conversion of the counter ion is carried out before the reaction solution is allowed to cool. This is advantageous because larger crystal sizes are produced in the precipitate which are easier to filter. Numerous "counter ions" can be used for this purpose, of which the most preferred are the nitrate, fluoroborate and methane sulphonate (PAAN, PAAFB and PAAMS for the acetato complex) along with the perchlorate. Other anions which may be used include the sulphate, carbonate and various phosphates along with a variety of organic anions including the acetate, glutamate, succinate, malonate, fumarate and toluene sulphonate. Typical organic anions include those of the formula R2 COO where R2 represents an optionally hydroxy substituted alkyl or alkenyl group 1 to 18, for example 1 to 6, carbon atoms. The presence of a longer hydrocarbon chain will add to the hydrophobicity of the complex which will be useful in certain applications. It will be appreciated that the aim is to obtain a good yield of the salt in a readily collectable form. The reaction conditions should be adjusted accordingly. The fluoroborate and methane sulphonate of the pentammonium acetate complex are believed to be novel and form another aspect of the present invention.
When nitrate is to be used as the new counter ion, nitric acid or a suitable nitrate salt (e.g. an alkali metal nitrate) may be used in the conversion reaction. Preferably the molar ratio of nitric acid or nitrate salt to cobalt(II) starting material is from 2:1 to 5:1, more preferably 2:1 to 3:1.
It will be appreciated that the use of less ammonia or amine than has been suggested in the past is beneficial both in terms of processing and in terms of effluent management. Thus effluent which contains less amino compounds presents less of an environmental hazard than effluent containing higher concentrations. Similar comments apply to the use of relatively small concentrations of hydrogen peroxide. This lower concentration aids safety since the addition of large quantities of hydrogen peroxide tends to cause an effervescence which give rise to high oxygen contents in the flue.
Although the present discussion principally concerns the acetato cobalt complexes it will be appreciated that similar comments apply to other carboxylato complexes obtained by using higher anhydrides such as propionic anhydride in place of acetic anhydride.
The following Examples farther illustrate the present invention.
The following material were used:
______________________________________ 32% ammonia solution 98-135 g (see Table) ammonium acetate 92 g 27% CoCl.sub.2 solution 190 g 35% H.sub.2 O.sub.2 solution 29 g 47% NaOH solution 97-100 g (see Table) Ac.sub.2 O 143 g Total 649-689 g ______________________________________
The ammonia solution and ammonium acetate were charged to a stirred flask equipped with a condenser; the temperature of the resulting solution was 12°-15° C. The cobalt chloride solution was added over 10-15 minutes resulting in an exothermal reaction which raised the temperature of the solution to 35°-46° C. (see Table). The peroxide solution was then added over 10-15 minutes resuking in an exotherm to approximately 60° C. The solution was heated to 65° C. and the sodium hydroxide was added over 15-20 minutes exotherming 1°-2° C. After stirring 30-45 minutes with a controller set at 65° C. PACC was no longer detected and the solution was cooled to approximately 25° C. and the acetic anhydride was added over 45-60 minutes with cooling applied to keep the temperature below 40° C. The details are given in Table 1.
TABLE 1 __________________________________________________________________________ pH Cobalt pH pH before Ammonia exo-therm/ before before NaOH Ac.sub.2 O Final % % Wt solution/g °C. H.sub.2 O.sub.2 NaOH solution/g (25° C.) pH Conversion PAAC __________________________________________________________________________ 98 35 8.5 7.5 99 10.9 4.6 80 13.2 107 34 8.7 8.0 98 10.9 4.7 85 13.8 115 43 8.65 8.0 100 10.9 4.75 83 13.7 135 46 8.9 8.4 97 11.0 5.1 75 11.9 __________________________________________________________________________
A bulk mixture was made from the solutions obtained. It analyzed as 13.7% Wt PAAC. It was used for precipitation trials. Three molar equivalents to Co of the acids shown in Table 2 were added to the solution with stirring; in each case an exotherm was observed. For nitrate and fluoroborate the slurry was gradually cooled to 5° C., filtered, washed with methanol and dried in a fan oven at 80° C. For methanesulphonate approximately 1.5 further mole equivalents of acid were added before precipitation started and the slurry treated as before. The overall yield assumes 85% conversion in solution.
TABLE 2 ______________________________________ % of soln Overall Assay as PAA yield from Solution Acid change Dry Yield PAAX isolated CoCl.sub.2 ______________________________________ 498 g 81 g 70% 82.0 g 98.8% 99.6 85% HNO.sub.3 PAAN 498 g 197 g 40% 79.5 g 97.1% 82.3 70% HBF.sub.4 PAAFB 353 g 130 g 70% 62.4 g 93.5% 84.0 71% MeSO.sub.3 H PAAMS ______________________________________
The nitrate and fluoroborate additions resulted in immediate precipitation i.e. with the first few drops. The nitrate and methanesulphonate products filtered readily in a few minutes whereas the fluoroborate was more difficult to isolate by vac-filtration, taking over an hour. In separate tests we found that the methanesulphonate product precipitated if less methanesulphonic acid was added so long as an addition of strong acid was made e.g. HCl We also found that the use of sodium fluoroborate solution as precipitant leads to a big improvement in the ease of isolation of the fluoroborate. We confirmed that the nitrate and fluoroborate could be washed with water; the methanesulphonate cannot be because it has a solubility of approximately 25% compared to <1% for PAAN and PAAFB at room temperature.
The following materials were used:
______________________________________ 32% ammonia solution 345 g ammonium acetate 300 g 27% CoCl.sub.2 solution 619 g 35% H.sub.2 O.sub.2 solution 95 g 47% NaOH solution 320 g Ac.sub.2 O 464 g (Sub-total 1) (2143 g) 70% HNO.sub.3 solution 234 g Reactor total 2377 g ______________________________________
The ammonia solution at 25° C. and ammonium acetate were charged to a stirred 31 RB Quickfit flask equipped with a condenser and reaction temperature-controller; after stirring 5 minutes the resulting solution registered 5° C. The cobalt chloride solution was added over 15 minutes in a steady stream resulting in an exotherm to 41° C. after approximately 3/4 of the addition; at the end of the addition the temperature in the flask was 38° C. After stirring 40 minutes the red solution was at 33° C. and registered pH 8.66; a trace of solid was observed in the flask. The hydrogen peroxide solution was added over 50 minutes during which time the temperature in the flask rose to 56° C. Early in the addition each drop produced a vigorous effervescence upon contact with the flask contents; towards the end the effervescence at the point of contact diminished significantly being replaced by a gentle effervescence across the surface and the solution developed a more intense red colour. The mantle was set to heat to 65° C.; at 60° C. the solution registered pH 7.9 and the caustic soda addition was started; it lasted 15 minutes during which time an exotherm was observed and the temperature peaked at 70° C. After stirring a further 30 minutes the temperature had dropped back to 65° C. and the solution registered pH 10.6 having peaked at 11.1; no solid was observed in the flask. After cooling to 27° C. the solution registered pH 11.2. The acetic anhydride was added over 110 minutes whilst the flask was immersed in a water bath (changed a few times); the maximum temperature observed was 38° C. After the addition there was no evidence of continuing exotherm and the pH was stable at 4.7. The solution was a deep red colour and no solid was observed in the flask. The flask was weighed and found to contain 2134 g nett, mass balance -9 g. A small sample was taken and analyzed by HPLC, <0.1% Wt. "PAC" was detected and the solution assayed as 14.8% "PAAC" (Conversion=88% on Co). The nitric acid solution was added at a steady rate over 35 minutes; an exotherm was observed as the flask contents rose to 45° C. with no cooling applied during the addition a red solid precipitated. The slurry was cooled to 23° C. over 60 minutes; it registered pH 3.5. It filtered with ease through a No1 porosity sintered-glass Buchner funnel under vacuum. The cake was washed with 2×approximately 200 mls ice cold water and left in the funnel for approximately 30 minutes.
Yield=2313 g combined liquor; 407 g wet-cake
The wet-cake was dried in a fan over at 80° C. for 2 hours, and ground in a mortar and pestle before analysis;
______________________________________ Yield = 351 g Assay = 100.2% as PAAN < 0.2% PAC i.e. 1.08 moles; 83% Yield on Cobalt. ______________________________________
The liquor registered pH 3.6. It was analyzed by HPLC and found to contain product equivalent to 20 g PAAN, i.e. 5% of Co charge. The nitric acid charge equates to 2 mole equivalents to Co, i.e. 2/3 the amount used in Example 1. In similar experiments from cobalt acetate we observed quantitative precipitation if the solutions were acidified to pH1; the pH drops rapidly below pH 3 so a small increase in nitric acid addition would probably maximise the yield. The liquor has a brown-black colour; it darkens during the nitric acid addition. It has a strong odor of acetic acid and the following approximate composition calculated by difference from the charges and dried product, assuming for the time being that "non-PAA cobalt" is present as HAC complex;
______________________________________ PAAN 0.06 moles 20 g 0.87% HAC 0.16 moles 59 g 2.5% sodium chloride 1.94 moles 113 g 4.9% sodium nitrate 0.44 moles 37 g 1.6% sodium acetate 1.42 moles 116 g 5.0% ammonium acetate 3.68 moles 283 g 12% acetic acid 6.8 moles 408 g 18% Total solids 1036 g 44.8% ______________________________________
The complexes contain 10 g cobalt i.e. 0.43% Wt. in the liquor.
The following materials were used:
______________________________________ 32% ammonia solution 398 g ammonium acetate 347 g 27% CoCl.sub.2 solution 714 g 35% H.sub.2 O.sub.2 solution 109 g 47% NaOH solution 370 g Ac.sub.2 O 536 g (Sub-total 1) (2474 g) 36% HCl solution 350 g 70% MeSO.sub.3 H solution 411 g Reactor total 3235 g ______________________________________
There were no significant differences to Example 2 up to the end of the anhydride addition when the flask contained 2461 g solution with pH 4.8 and an assay of 14.9% PAAC i.e. 89% conversion from Cobalt.
With the flask contents at 26° C. the hydrochloric acid addition was made over 20 minutes whilst cooling in a water bath to 24° C. when the solution registered pH 3.5. The methanesulphonic acid solution was added over 45 minutes accompanied by a raise in temperature in the flask to 29° C. and a drop in pH to <1. After approximately 80% of the addition the product "dropped out" of solution and an exotherm was observed to 34° C. After cooling to 15° C. the slurry was filtered through two No1 porosity sintered-glass Buchner funnels under vacuum, the cake was washed with a total of 600 mls methanol and left in the funnel overnight then dried for an hour in a fan oven at 80° C., and ground in a mortar and pestle before analysis.
Yield=2313 g combined liquor; 440 g Dry product
Assay=97.1% as PAAMS, approximately 3% "PAC"
i.e. 1.09 moles; 84% Yield on Cobalt.
A batch of solution was prepared as for PAAMS (Example 3) with c. 3.5 hours for the anhydride addition. The yield was 2481 g with pH 4.83 and assay 14.6% PAAC, i.e. 88% conversion.
The desired product was made by sodium fluoroborate precipitation and water washing from a composite sample of "PAA" solutions prepared in the presence of chloride and acetate ions, i.e. samples from both cobalt salts+"opposite" buffering add. The "PAA" solution assayed 13.0% as PAAC and contained practically no PACC. The percentage yield for this step was 70%, i.e. percentage of solution "PAA" found in the washed and dried PAAFB; 239 g Dry product; Assay=101% as PAAFB, <0.2% "PAC".
A series of experiments were performed on cobalt (II) acetate tetrahydrate with ammonium chloride at the same pH's and temperatures as in Example 1. The conversions were not as good even if water was added to the same overall strength, namely 66% conversion using `all-crystals` and 75% with added water (either as cobalt acetate solution, or diluted ammonia reactants+cobalt acetate crystals). The pH's after acetic anhydride addition were approximately 4.5 as expected.
Further experiments were performed at 8 moles total ammonia species per mole cobalt with other acid buffers to give solutions of Co (II) complexes with pH approximately 8.7 prior to oxidation:
______________________________________ Cobalt (II) salt Acid Moles ammonia Moles amm. salt ______________________________________ Chloride HCl 5.7 2.3 Chloride AcOH 5.0 3.0 Acetate HCl 5.4 2.6 Acetate AcOH 4.0 4.0 Acetate H.sub.2 SO.sub.4 5.2 1.4 Acetate MeSO.sub.3 H 5.85 2.15 Acetate HNO.sub.3 4.5 3.5 ______________________________________
Following the same method as before with all acetate species the following results were obtained;
______________________________________ Moles Ac.sub.2 O:Co pH % Conversion ______________________________________ 3 5.6 61 3/5 5.6 75 5 5 78 ______________________________________
Experiments with 3 moles anhydride and sulphate or methanesulphonate buffering prepared in-situ resulted in conversions of 61 and 59% respectively in solutions of pH 4.7 and 4.65. Experiments with ammonium nitrate, added as solid, resulted in precipitation of product as `PAA` formed; the final mixtures were acidified to pH 1 when PAAN was collected quantitatively, i.e. no `PAA` remained in the liquors. The best yield was 69% from 3 moles anhydride; the slurry prior to nitric acid addition registered pH 4.8.
The following material was used:
______________________________________ Ammonium acetate 162 g 28% Ammonia Solution 233 g Cobalt (II) acetate.4H.sub.2 O 87 g 35% H.sub.2 O.sub.2 34 g (Solution sub-total) (516 g) 45% NaNO.sub.3 265 g Total 781 g ______________________________________
Cobalt acetate was quickly added to freshly prepared ammonia buffer at 11° C. to form a clear solution at a temperature of 26° C. The hydrogen peroxide solution was then added over 20 minutes without cooling during which time the temperature of the solution rose from 26° C. to 49° C. The solution was then stirred for one hour. After stirring, the temperature of the solution was 33° C. It was then heated to a temperature of 80° C. It was then maintained at this temperature for six hours. After cooling to 21° C., the sodium nitrate solution was added over a period of 20 minutes. 20 minutes after the addition of the sodium nitrate solution, the solution was cooled and after an hour, it was filtered and washed with iced water. The product filtered slowly and gave a very wet cake (approximately 30% water) which was dried in an oven at 70° C.
The mass balance showed that 83 g was lost per mole of cobalt. The conversion of cobalt based on the mount of PAAA obtained was 90.5%. In the assay of the dry product was found 96.7% by weight of PAAN and 3.9% by weight of HAN ( CoIII (NH3)6 !(NO3)3). The dry yield of PAAN with respect to the mount of cobalt used was 86%. The recovery of PAA from solution was 95%.
The following material was used:
______________________________________ Ammonium acetate 578 g 28% Ammonia solution 835 g Cobalt (II) acetate.4H.sub.2 O 311 g Solution total 1724 g ______________________________________
Cobalt acetate was added quickly to freshly prepared ammonia buffer without cooling. The resultant solution was dear and had a temperature of 23° C. Air was then bubbled through the solution at a rate of 800 ml/min and was left on overnight. After approximately 20 hours, the air supply was stopped and the solution was heated to 80° C. and this temperature was maintained for six hours. At the end of the heating, the solution was cooled.
The mass balance showed that 94 g was lost per mole of cobalt in the experiment. The conversion rate of cobalt based on the PAAA assay was 85.8%.
The following material was used:
______________________________________ Ammonium acetate 216 g 32% Ammonia solution 234 g Cobalt (II) acetate.4H.sub.2 O 199 g 35% hydrogen peroxide 58 g Solution total 707 g ______________________________________
Cobalt acetate was added to freshly prepared ammonia buffer quickly without cooling. The resultant solution was clear and had a temperature of 28° C. Peroxide solution was then added over a period of 50 minutes without cooling. The resultant solution which had a temperature of 59° C. was then stirred for 40 minutes. The stirred solution was heated to 80° C. and this temperature was maintained for six hours. The solution was then cooled.
The mass balance showed that 5 g was lost per mole of cobalt in the experiment. The conversion rate of cobalt based on the PAAA assay was 88.9%.
The following material was used:
______________________________________ Ammonium acetate 1011 g 32% Ammonia solution 1095 g Cobalt (II) acetate.4H.sub.2 O 934 g 35% hydrogen peroxide 219 g Solution total 3259 g ______________________________________
Cobalt acetate was added to freshly prepared ammonia buffer quickly without cooling. The resultant solution had a temperature of 26° C. and after 60 minutes, the hydrogen peroxide solution was added over a period of 33/4 hours. Frothing was observed towards the end of the peroxide addition and water was used to wash down the condenser. After the addition of peroxide, the solution was maintained at a temperature of 46° C. for 20 minutes. It was then heated to 80° C. and maintained over night before being cooled.
The conversion rate of cobalt based on the PAAA assay was 86.4%.
The following material was used:
______________________________________ Ammonium acetate 606 g 28% Ammonia Solution 657 g Cobalt (II) acetate.4H.sub.2 O 560 g Solution total 1823 g ______________________________________
Cobalt acetate was added to freshly prepared ammonia buffer quickly without cooling. The resultant solution was clear and had a temperature of 27° C. After 55 minutes, air was bubbled through the solution at a rate of 1800 ml/min and the air was left on overnight. Approximately 20 hours later, the air supply was stopped and the solution was heated to 80° C. and maintained at this temperature for 6 hours before being cooled.
The mass balance showed that 32 g was lost per mole of cobalt in the experiment. The conversion rate of cobalt based on the PAAA assay was 70.0%.
The following material was used:
______________________________________ Example 9 solution 436 g 45% sodium nitrate 189 g (First aliquot) 45% sodium nitrate 66 g (Second aliquot) Slurry total 691 g ______________________________________
The first aliquot of sodium nitrate was added over a period of 55 minutes without cooling. Precipitation started with the first few drops and was mildly exothermic. The final temperature of the solution was 30° C. and an assay of the supernatant after addition of the first aliquot showed that less than 5% of PAA remained in the solution. The second aliquot of sodium nitrate was then added after a wait of 35 minutes over a period of 15 minutes. An assay of the supernatant after the addition of the second aliquot showed that an insignificant mount of PAA remained in the solution. After one hour, the precipitate was filtered and washed with 200 ml of ice water.
In the assay of the dry product was found 92.7% by weight of PAAN and 6.5% by weight of HAN. The dry yield of PAAN with respect to the amount of cobalt used was 82%. The recovery of PAA from solution was 95%.
The following material was used:
______________________________________ Example 9 solution 523 g 68% nitric acid 111 g 68% nitric acid 39 g Slurry total 673 g ______________________________________
The first aliquot of nitric acid was added over a period of 20 minutes without cooling. Precipitation started with the first few drops and was highly exothermic. The final temperature was 59° C. An assay of the supernatant after the addition of the first aliquot showed that less than 5% of PAA remained in the solution. Cooling was then applied for 1/2 hour until a temperature of 18° C. was reached and then the second aliquot was added over a period of 10 minutes. An assay of the supernatant after the addition of the second aliquot showed that an insignificant trace of PAA remained in the solution. The product was cooled for 40 minutes then filtered and washed with 240 ml iced water.
In the assay of the dry product was found 94.6% by weight of PAAN and 6.8% by weight of HAN. The dry yield of PAAN with respect to the amount of cobalt used was 86%. The recovery of PAA from solution was 99.5%.
Claims (15)
1. A process for preparing a cobalt III complex which comprises:
(i) treating a divalent cobalt salt of formula CoII X2/n where n is the valency of an anion X, with up to 15 molar equivalents of ammonia or an amine;
(ii) oxidising the resulting amine complex;
(iii) converting the oxidised complex to the corresponding carboxylate of formula CoIII (NR3)5 R1 COO!X2/n where each R, which may be the same or different, represents hydrogen or an optionally substituted hydrocarbon group and R1 represents an alkyl or alkenyl group of 1 to 18 carbon atoms, at a pH above 8.5; and optionally
(iv) replacing the X ion by a different anion by a metathetical reaction.
2. A process according to claim 1 in which the divalent cobalt salt is cobaltous acetate.
3. A process according to claim 1 or 2 in which ammonia is used in step (i).
4. A process according to claim 3 in which the ammonia is added as ammonium acetate.
5. A process according to claim 4 in which the molar ratio of ammonia to cobalt salt is from 5:1 to 6:1.
6. A process according to claim 4 in which the molar ratio of ammonium salt to the cobalt salt is from 3:1 to 4:1.
7. A process according to claim 1 in which step (ii) is carried out with hydrogen peroxide.
8. A process according to claim 7 in which the hydrogen peroxide is used in an amount from 0.5 to 1 moles per mole of complex.
9. A process according to claim 1 in which after step (ii) and before (iii) the pH is raised to 9 to 12 by the addition of alkali metal hydroxide and/or ammonium hydroxide.
10. A process according to claim 1 in which step (iii) is carried out using the corresponding carboxylic acid anhydride of formula (R1 CO)2 O.
11. A process according to claim 1 in which R represents methyl.
12. A process according to claim 1 in which step (iv) is carried out wherein the new ion X is the nitrate, fluoroborate, methane sulphonate or perchlorate.
13. A cobalt complex of the formula CoIII (NR3)5 R1 COO!X2/n where each R, which may be the same or different, represents hydrogen or an unsubstituted or substituted hydrocarbon group, R1 represents methyl, X represents fluoroborate or methane sulphonate and n is the valency of X.
14. A process according to claim 3 in which the molar ratio of ammonia to cobalt salt is from 5:1 to 6:1.
15. A process according to claim 3 in which the molar ratio of ammonium salt to the cobalt salt is from 3:1 to 4:1.
Applications Claiming Priority (5)
Application Number | Priority Date | Filing Date | Title |
---|---|---|---|
GBGB9516683.1A GB9516683D0 (en) | 1995-08-15 | 1995-08-15 | Cobalt catalyst |
GB9516683 | 1995-08-15 | ||
GB9604721A GB2310852B (en) | 1996-03-05 | 1996-03-05 | Carboxylatocomplexes of Cobalt |
GB9604721 | 1996-03-05 | ||
PCT/GB1996/001986 WO1997007124A1 (en) | 1995-08-15 | 1996-08-14 | Improved cobalt catalyst |
Publications (1)
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US5739367A true US5739367A (en) | 1998-04-14 |
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ID=26307570
Family Applications (1)
Application Number | Title | Priority Date | Filing Date |
---|---|---|---|
US08/817,295 Expired - Lifetime US5739367A (en) | 1995-08-15 | 1996-08-14 | Cobalt catalyst |
Country Status (6)
Country | Link |
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US (1) | US5739367A (en) |
EP (1) | EP0785940B1 (en) |
AT (1) | ATE214706T1 (en) |
DE (1) | DE69619958T2 (en) |
ES (1) | ES2173309T3 (en) |
WO (1) | WO1997007124A1 (en) |
Cited By (1)
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US6911485B1 (en) * | 2002-04-19 | 2005-06-28 | The University Of Georgia Research Foundation, Inc. | Anionic and Lewis base photopolymerization process and its use for making optical articles |
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AU2002300321B2 (en) * | 1998-05-18 | 2005-05-19 | Robert Andrew Crosbie | Chair and seat cushion therefor |
PH11999002190B1 (en) * | 1998-09-01 | 2007-08-06 | Unilever Nv | Composition and method for bleaching a substrate |
PH11999002188B1 (en) * | 1998-09-01 | 2007-08-06 | Unilever Nv | Method of treating a textile |
BR0013745A (en) | 1999-09-01 | 2002-05-14 | Unilever Nv | Bleaching composition for a textile |
BR0013592A (en) | 1999-09-01 | 2002-05-07 | Unilever Nv | Commercial packaging for bleaching fabric stains in an aqueous washing liquor, and using it |
GB0004990D0 (en) | 2000-03-01 | 2000-04-19 | Unilever Plc | Composition and method for bleaching a substrate |
BR0013593A (en) | 1999-09-01 | 2002-05-07 | Unilever Nv | Method for bleaching fabric stains |
BR0108772A (en) | 2000-02-29 | 2002-11-26 | Unilever Nv | Bleaching composition, method for bleaching a substrate, and, binding |
Citations (3)
Publication number | Priority date | Publication date | Assignee | Title |
---|---|---|---|---|
GB2034061A (en) * | 1978-09-27 | 1980-05-29 | Fuji Photo Film Co Ltd | Silver halide colour photographic lightsensitive material |
US5559261A (en) * | 1995-07-27 | 1996-09-24 | The Procter & Gamble Company | Method for manufacturing cobalt catalysts |
US5581005A (en) * | 1995-06-16 | 1996-12-03 | The Procter & Gamble Company | Method for manufacturing cobalt catalysts |
-
1996
- 1996-08-14 WO PCT/GB1996/001986 patent/WO1997007124A1/en active IP Right Grant
- 1996-08-14 DE DE69619958T patent/DE69619958T2/en not_active Expired - Lifetime
- 1996-08-14 AT AT96927783T patent/ATE214706T1/en not_active IP Right Cessation
- 1996-08-14 US US08/817,295 patent/US5739367A/en not_active Expired - Lifetime
- 1996-08-14 EP EP96927783A patent/EP0785940B1/en not_active Expired - Lifetime
- 1996-08-14 ES ES96927783T patent/ES2173309T3/en not_active Expired - Lifetime
Patent Citations (3)
Publication number | Priority date | Publication date | Assignee | Title |
---|---|---|---|---|
GB2034061A (en) * | 1978-09-27 | 1980-05-29 | Fuji Photo Film Co Ltd | Silver halide colour photographic lightsensitive material |
US5581005A (en) * | 1995-06-16 | 1996-12-03 | The Procter & Gamble Company | Method for manufacturing cobalt catalysts |
US5559261A (en) * | 1995-07-27 | 1996-09-24 | The Procter & Gamble Company | Method for manufacturing cobalt catalysts |
Non-Patent Citations (6)
Title |
---|
Jackman et al., "Synthesis of Transition-Metal Carboxylato Complexes1,2 ", Inorganic Chemistry, 18(6):1497-1502 (1979). |
Jackman et al., Synthesis of Transition Metal Carboxylato Complexes 1,2 , Inorganic Chemistry, 18(6):1497 1502 (1979). * |
Kirschner et al., "The Effects of Ion Association on the Optical Rotary Dispersion of Coordination Compounds", Chemical Abstracts, 64(13):18452a (1966). |
Kirschner et al., The Effects of Ion Association on the Optical Rotary Dispersion of Coordination Compounds , Chemical Abstracts, 64(13):18452a (1966). * |
Wierenga et al., "Synthesis and Characteristics of Cobalt(III) Nicotinic Acid Complexes", Inorganic Chemistry, 21:2881-2885 (1992). |
Wierenga et al., Synthesis and Characteristics of Cobalt(III) Nicotinic Acid Complexes , Inorganic Chemistry, 21:2881 2885 (1992). * |
Cited By (3)
Publication number | Priority date | Publication date | Assignee | Title |
---|---|---|---|---|
US6911485B1 (en) * | 2002-04-19 | 2005-06-28 | The University Of Georgia Research Foundation, Inc. | Anionic and Lewis base photopolymerization process and its use for making optical articles |
US20050203200A1 (en) * | 2002-04-19 | 2005-09-15 | Kutal Charles R. | Anionic and Lewis base photopolymerization process and its use for making optical articles |
US7253213B2 (en) * | 2002-04-19 | 2007-08-07 | Kutal Charles R | Anionic and Lewis base photopolymerization process and its use for making optical articles |
Also Published As
Publication number | Publication date |
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ES2173309T3 (en) | 2002-10-16 |
EP0785940B1 (en) | 2002-03-20 |
EP0785940A1 (en) | 1997-07-30 |
ATE214706T1 (en) | 2002-04-15 |
WO1997007124A1 (en) | 1997-02-27 |
DE69619958T2 (en) | 2002-10-02 |
DE69619958D1 (en) | 2002-04-25 |
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